Calculate the change in the standard free energy for the following reaction: Znc+Cu?" (aq) (a +...
+ Calculate the change in the standard free energy for the following reaction: Zn + Cu?+ Zn²+ (aq) + Cu (3) Standard Reduction Potentials (5) (aq) + 2e → = -0.763 V (aq) + 2e → Cu (s) Ered = 0.337 V (aq) → → Zn (5) Ered Zn2+ Cu2+ A. - 212 kJ/mol B. 175 kJ/mol C. 81.0 kJ /mol OD. - 106 kJ / mol
Please circle final answer Calculate the change in free energy (AG) for the following standard cell between Barium and Copper. Recall AG = -nFEcell, and F = 9.65 x 10 C/mol Ba Ba2 (aq) + 2e, E red -2.90 V 2e+Cu2+ (aq) Cus), Ered = +0.337 V +625 kJ/mol +495 kJ/mol -625 kJ/mol 495 kJ/mol
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
1. Some standard reduction potentials at 25 C are: E 0.337 V for Cu* (a) 2e- Cu(s) E" =-0.1 26 V for Phẩ (aq) + 2e → Pb(s) Eo-0.763 V for Zn2 (a)2e-> Zn(s) Predict the voltage of each of the following voltaic cells: a. Cu | Cu0.010 M)I Cu (0.010M) | Cu c. Zn | Zn2 (0010 M) Cu(0.010 M) | Cu b. Pb | Pb (0.010 M)1 Cu (0.010 MCud. Zn | Zn3 (0.010 M) 11 Pb (0.010...
Constants The following values may be useful when solving this tutorial. Constant Value E∘Cu 0.337 V E∘Zn -0.763 V R 8.314 J⋅mol−1⋅K−1 F 96,485 C/mol T 298 K Part A Part complete In the activity, click on the E∘cell and Keq quantities to observe how they are related. Use this relation to calculate Keq for the following redox reaction that occurs in an electrochemical cell having two electrodes: a cathode and an anode. The two half-reactions that occur in the...
Consider the following cell reaction at 18°C: Ca(e)+Cu+ (aq) + Ca2+ (aq) + Cu() Calculate the standard cell potential of this cell from the standard electrode potentials, and from this, obtain AG" for the cell reaction. Calculate AF. Use these values of AN and AG to obtain AS for the cell reaction. Ca²+ (aq) +20 + Ca() --2.76 V Cu? (g) +20 + Cu(s) - 0.84 V AH;(O.*()) -- 542.8 kJ/mol AH;(Out (as)) - 64.8 kJ/mol V AG- AH- kJ...
CU PIULUOS LO UCCU 30. Based on the given standard free energy change and electron stoichiometry values below, calculate a corresponding standard cell potential. AG°= 12 kJ/mol, n=3 A. Eceu=0.041 V B. Eceu= +0.047 V C. Eceu=-0.041 V D. Eceu= -0.047 V
The free energy change for the following reaction at 25 °C, when [Cr3+] = 6.08×10-3 M and [Cu2+] = 1.12 M, is 67.3 kJ: Cr3+(6.08×10-3 M) + Cu+(aq) Cr2+(aq) + Cu2+(1.12 M) ΔG = 67.3 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
The free energy change for the following reaction at 25 °C, when Cu?) - 1.15 M and Co2+) = 3.46x10-M, is -133 kJ: Cu2+(1.15 M) + Co(s) — Cu(s) + Co2+(3.46x10-3 M) AG --133 kJ What is the cell potential for the reaction as written under these conditions? Answer: V Would this reaction be spontaneous in the forward or the reverse direction?
Calculate the standard free-energy change at 25 ∘C for the following reaction: Mg2+(aq) + Zn(s) → Mg(s) + Zn2+(aq) Express your answer to three significant figures and in units of kJ/mol. Consider constructing a voltaic cell with one compartment containing a Zn(s) electrode immersed in a Zn2+ aqueous solution and the other compartment containing an Al(s) electrode immersed in an Al3+ aqueous solution. What is the spontaneous reaction in this cell? Group of answer choices Zn + Al3+ → Al...